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16-September-2008 16:20:32 - Peroxide For other uses, see Peroxide disambiguation. A peroxide is a compound containing an oxygen-oxygen single bond. The simplest stable peroxide is hydrogen peroxide. Superoxides, dioxygenyls, ozones and ozonides compound are considered separately. Organic chemistry Main article: Organic peroxide In organic chemistry, peroxide is a specific functional group or a molecule containing an oxygen-oxygen single bond R-O-O-R'. When the other oxygen bears a hydrogen, it is called a hydroperoxide R-O-O-H. The radical HOO· is known as hydroperoxide radical, and is thought to be involved in combustion of hydrocarbons in air. Organic peroxides tend to decompose easily to free radicals of the form: RO· This makes them useful as catalysts for some types of polymerisation, such as the polyester resins used in glass-reinforced plastics. MEKP methyl ethyl ketone peroxide is commonly used for this purpose. However, the same property also means that organic peroxides can accidentally initiate explosive polymerization in materials with unsaturated chemical bonds. Since peroxides can form spontaneously in some materials, some caution must be exercised with such peroxide-forming materials. Triacetone triperoxide TATP and hexamethylene triperoxide diamine are explosive organic peroxide compounds; TATP may be formed accidentally as a waste product in some reactions. In addition, many liquid ethers in the presence of air, light, and metal slowly over a period of months form ether peroxides e.g., diethyl ether peroxide, which are extremely unstable. As a consequence, it is recommended that ether be stored over potassium hydroxide, which not only destroys peroxides but also acts as a powerful desiccant. Extreme care must be taken with samples showing signs of crystal growth or precipitates. TATP is an easily synthesized, inexpensive, explosive compound that is difficult to detect by normal screening methods. Consequently, it is an explosive favored by terrorists. TATP was used in the 2005 London Underground bombings and the 2001 shoe bomber. In 2002, a simple mass spectroscopy screening method was developed.1 Inorganic chemistry In inorganic chemistry, peroxide is the anion O22-. It is highly basic, and present in ionic compounds. Pure peroxides containing only cations and the peroxide anions are usually formed by burning alkali metals or alkaline earth metals in air or oxygen. Sodium peroxide Na2O2 is a typical example. The peroxide ion contains two electrons more than the oxygen molecule. These two electrons, according to the molecular orbital theory, complete the two Ï€ antibonding orbitals. This has as result a weakening of the bond strength of the peroxide ion and a greater length for the bond O-O : Li2O2 130 pm to BaO2 147 pm. Furthermore, the peroxide ion is diamagnetic. The peroxides of the alkali metals and Ca, Sr and Ba are ionic. The peroxides of a number of electropositive metals such as Mg, the lanthanides and the uranyl-ion show an intermediary character, between ionic and covalent. The peroxides of metals such as Zn, Cd and Hg are mainly covalent. Peroxides are powerful oxidizers, and usually fairly unstable. Ionic peroxides react with water and diluted acids to form hydrogen peroxide. Organic compounds are oxidized to carbonates, even at normal temperatures. Sodium peroxide is a powerful oxidator of metals, such as iron. The oxides, peroxides and superoxides are closely related, forming a chain of oxygen ions of progressively higher oxidation number. Barium peroxide is used in pyrotechnics and tracer ammunition, and was once used in the manufacture of hydrogen peroxide. Sodium peroxide is used as a carbon dioxide absorber and oxygen regenerator e.g. in some submarines, through the reaction: 2Na2O2 + 2CO2 → 2Na2CO3 + O2 See also catalase oxygen ozone peroxidases hydrogen peroxide carbamide peroxide sodium percarbonate calcium peroxide magnesium peroxide potassium monopersulfate sodium perborate monohydrate ozonide, O3- superoxide, O2- oxide, O2- dioxygenyl, O2+ v d e Functional groups Chemical class: Alcohol Aldehyde Alkane Alkene Alkyne Amide Amine Azo compound Benzene derivative Carboxylic acid Cyanate Disulfide Ester Ether Haloalkane Hydrazone Imine Isocyanide Isocyanate Ketone Oxime Nitrile Nitro compound Nitroso compound Peroxide Phosphoric acid Pyridine derivative Sulfone Sulfonic acid Sulfoxide Thioester Thioether Thiol Retrieved from http://en..org/wiki/Peroxide Categories: Anions | Oxygen compounds | Peroxides Views Article Discussion this page History Personal tools Log in / create account Navigation Main page Contents Featured content Current events Random article Search Go Search Interaction Community portal Recent changes Contact Donate to Help Toolbox What links here Related changes Upload file Special pages Printable version Permanent link Cite this page Languages Bosanski Deutsch Español Français Hrvatski Bahasa Indonesia Italiano Lietuvių Nederlands 日本語 Plattdüütsch Polski Português РуÑ?Ñ?кий СрпÑ?ки / Srpski Srpskohrvatski / СрпÑ?кохрватÑ?ки Suomi Svenska УкраїнÑ?ька ä¸æ–‡ This page was last modified on 31 July 2008, at 06
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